Reaction Rate Vs

Lab-Types of Reactions

Purpose: In this experiment, you will investigate the general characteristics of the five types of reactions that make up one of the schemes used to classify chemical reactions. You will observe examples of combination, decomposition, single replacement, double replacement and combustion reactions. You will then balance the equations for these reactions.

Materials: Mg metal steel wool 3 M HCl Bunsen burner

0.1 M CuSO4 test tubes(large and small)

NH3 wooden splint

CuCO3 test tube holder

0.1 M Pb(NO3)2 crucible tongs

1 M K2CrO4

Procedure: Reaction 1 Reaction of magnesium metal with a solution of hydrochloric acid: 1. Place approximately 15 drops of 3 M HCl in a clean, thoroughly dry test tube. 2. Add a piece of Mg metal ribbon to the 3 M HCl in the test tube. Allow the test tube to stand for several minutes. Record your observations in your data table. 3. Dispose of the material in the test tube by flushing it down the drain with tap water. 4. Rinse the test tube thoroughly with tap water. Reaction 2 Reaction of a solution of copper(II) sulfate with aqueous ammonia.

1. Place 10 drops of 0.1 M CuSO4 in a clean, thoroughly dry small test tube.

2. Add 5 drops of NH3 to the 0.1 M CuSO4 in the test tube and gently mix the chemicals. Record your observations in your data table. 3. Dispose of the material in the test tube by flushing it down the drain with tap water. Reaction 3 Reaction of copper (II) carbonate

1. Measure about 1 g of CuCO3 on a piece of creased paper. Carefully pour the CuCO3 into a large test tube. 2. Hold the test tube at a slight incline with a test tube holder and gently heat in a flame for about one minute. Then, heat the test tube strongly for an additional two minutes. Immediately insert a burning wood splint into the test tube. Record your observations in your data table. 3. Dispose of the wooden splint in the trash. Thoroughly clean the test tube with tap water and flush the contents down the drain. Reaction 4 Reaction of a solution of lead(II) nitrate with a solution of potassium chromate

1. Place 10 drops of 0.1 M Pb(NO3)2 in a clean thoroughly dry small test tube.

2. Add 5 drops of 1 M K2CrO4 to the 0.1 M Pb(NO3)2 in the test tube and gently mix the chemicals. Record your observations in your data table. 3. Dispose of the material in the test tube by flushing it down the drain with tap water. 4. Rinse the test tube thoroughly with tap water.

Reaction 5 Reaction of iron metal(steel wool) with oxygen gas 1. Fluff up a small sample of steel wool until it is a sphere approximately an inch in diameter. 2. Using a pair of crucible tongs, hold the sphere of steel wool in a Bunsen burner flame for a few seconds. Then take it out an note what happens. Record your observations in your data table. 3. Dispose of any unreacted steel wool in a waste basket.

Data and Analysis: Complete the following summary table by recording your observations and the evidence from the experiment that a chemical change took place.

Reaction Observation Evidence of Chemical Change 1 2 3 4 5

Conclusion: 1. Write a balanced chemical equation for Reaction 1. Note: The acid used in this reaction is a diluted aqueous solution.

2. For Reaction 2, the aqueous reactants produced tetraamine copper sulfate, Cu(NH3)4SO4 (found in an aqueous solution.) Write a balanced chemical equation for this reaction. 3. For Reaction 3, the reactant decomposed into solid copper(II) oxide and carbon dioxide gas. Write a balanced chemical equation for this reaction. 4. Write a balanced chemical equation for Reaction 4. Note: Both reactants are in aqueous solutions.

5. For Reaction 5, when the iron reacts with oxygen gas, solid magnetite, Fe3O4 is produced. Write a balanced chemical equation for this reaction. 6. Identify the type of reaction that took place for: a. Reaction 1 b. Reaction 2 c. Reaction 3 d. Reaction 4 e. Reaction 5

Grading Data and Analysis: Complete the following summary table by recording your observations and the evidence from the experiment that a chemical change took place.

Reaction Observation Evidence of Chemical Change 1 2 3 4 5

Conclusion: 1. Write a balanced chemical equation for Reaction 1. Note: The acid used in this reaction is a diluted aqueous solution.

2. For Reaction 2, the aqueous reactants produced tetraamine copper sulfate, Cu(NH3)4SO4 (found in an aqueous solution.) Write a balanced chemical equation for this reaction.

3. For Reaction 3, the reactant decomposed into solid copper(II) oxide and carbon dioxide gas. Write a balanced chemical equation for this reaction.

4. Write a balanced chemical equation for Reaction 4. Note: Both reactants are in aqueous solutions.

5. For Reaction 5, when the iron reacts with oxygen gas, solid magnetite, Fe3O4 is produced. Write a balanced chemical equation for this reaction.

6. Identify the type of reaction that took place for: a. Reaction 1 b. Reaction 2 c. Reaction 3 d. Reaction 4 e. Reaction 5